In the complete combustion of C3H8 (propane), how many liters of CO2 are produced from 10 liters of O2?
C3H8 + 5O2 ==> 3CO2 + 4H2O
10 L O2 x (3 mols CO2/5 mols O2) = 10 L x 3/5 = ?
the balanced equation reveals the answer
C₃H₈ + 5 O₂ ---> 3 CO₂ + 4 H₂O
looks like 6
To determine the number of liters of CO2 produced from the complete combustion of propane (C3H8) using 10 liters of O2, we first need to calculate the balanced chemical equation for the reaction.
The balanced chemical equation for the complete combustion of propane is as follows:
C3H8 + 5O2 -> 3CO2 + 4H2O
From the balanced equation, we can see that the molar ratio between oxygen (O2) and carbon dioxide (CO2) is 5:3. This means that for every 5 moles of O2, we get 3 moles of CO2.
Since we are given the volume of O2 (10 liters), we need to convert it to moles. To do this, we can use the ideal gas law:
PV = nRT
Where:
P = pressure (assumed constant)
V = volume (in liters)
n = number of moles
R = ideal gas constant
T = temperature (assumed constant)
Assuming pressure and temperature are constant, we can simplify the equation to:
V = n
Therefore, the 10 liters of O2 is equal to 10 moles of O2.
Now, since the molar ratio between O2 and CO2 is 5:3, we can set up a ratio:
5 moles O2 : 3 moles CO2
Using the ratio, we can calculate the number of moles of CO2 produced:
10 moles O2 x (3 moles CO2 / 5 moles O2) = 6 moles CO2
Finally, to convert moles to liters, we can use Avogadro's law, which states that equal volumes of ideal gases at the same temperature and pressure contain an equal number of molecules:
1 mole of gas = 22.4 liters (at standard temperature and pressure)
Therefore, the number of liters of CO2 produced would be:
6 moles CO2 x 22.4 liters/mole = 134.4 liters CO2
So, from 10 liters of O2, approximately 134.4 liters of CO2 would be produced in the complete combustion of propane.
To determine the number of liters of CO2 produced from 10 liters of O2 during the complete combustion of C3H8 (propane), we need to understand the balanced chemical equation for the combustion reaction.
The balanced equation for the complete combustion of propane is:
C3H8 + 5O2 → 3CO2 + 4H2O
From the balanced equation, we can see that for every 5 moles of O2, we get 3 moles of CO2.
Given that we have 10 liters of O2, we need to convert the volume to moles. To do this, we need to know the molar volume of O2 at the given conditions (e.g., temperature and pressure). Assuming standard temperature and pressure conditions (STP), 1 mole of any ideal gas occupies 22.4 liters of volume.
Therefore, 10 liters of O2 can be converted to moles by dividing by the molar volume:
10 liters O2 / 22.4 liters/mole = 0.4464 moles of O2
Now that we have the moles of O2, we can determine the moles of CO2 produced by using the mole ratio from the balanced equation. From the equation, we know that:
5 moles of O2 produces 3 moles of CO2
Using this ratio, we can calculate the moles of CO2 produced:
0.4464 moles O2 * (3 moles CO2 / 5 moles O2) = 0.26784 moles CO2
Finally, we need to convert the moles of CO2 back to liters by multiplying by the molar volume:
0.26784 moles CO2 * 22.4 liters/mole = 5.987 liters CO2
Therefore, the complete combustion of 10 liters of O2 in the presence of propane (C3H8) would produce approximately 5.987 liters of CO2.